1. The equilibrium constant, K, for a redox reaction is related to the standard potential, E∘, by the equation ln K=nFE∘

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1. The equilibrium constant, K, for a redox reaction is
related to the standard potential, E∘, by the equation
ln K=nFE∘RT, where n is the number of moles of electrons
transferred, F (the Faraday constant) is equal
to 96,500 C/(mol e−)C/(mol e−), R (the
gas constant) is equal to 8.314 J/(mol⋅K),
and T is the Kelvin temperature.
Calculate the standard cell potential (E∘E∘) for the
reaction
X(s)+Y+(aq)→X+(aq)+Y(s)
if K = 9.10×10−4.
Express your answer to three significant figures and include the
appropriate units.
2. Calculate the standard cell potential at
25 ∘C∘C for the reaction
X(s)+2Y+(aq)→X2+(aq)+2Y(s)
where ΔH∘ = -655 kJand ΔS∘ = -253 J/K
Express your answer to three significant figures and include the
appropriate units.